AP Chemistry · Unit 7
Equilibrium
In short
Unit 7: Equilibrium in AP Chemistry covers 12 topics: Introduction to Equilibrium, Direction of Reversible Reactions, Reaction Quotient and Equilibrium Constant, Calculating the Equilibrium Constant and 8 more. Open each one for what you need to know, a self-check list and how it is tested on the exam.
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What is in Unit 7: Equilibrium?
Unit 7: Equilibrium
7.1 Introduction to Equilibrium
- I can explain the relationship between a reversible process and the establishment of equilibrium using experimental observations.
- I can identify examples of reversible physical and chemical processes, such as phase changes, dissolution, acid-base reactions, and redox reactions.
- I can recognize that at equilibrium, no observable changes occur, both reactants and products are present, and their concentrations or partial pressures remain constant.
- I can describe the dynamic nature of equilibrium, where forward and reverse processes occur at equal rates.
- I can interpret graphs of concentration, partial pressure, or rate of reaction versus time to determine when chemical equilibrium is established.
7.2 Direction of Reversible Reactions
7.3 Reaction Quotient and Equilibrium Constant
7.4 Calculating the Equilibrium Constant
7.5 Magnitude of the Equilibrium Constant
7.6 Properties of the Equilibrium Constant
- I can invert the value of K when a chemical reaction is reversed.
- I can calculate the K of an overall reaction by multiplying the K values of the individual reactions that were summed together.
- I can apply all valid algebraic manipulations of K to the reaction quotient Q.
7.7 Calculating Equilibrium Concentrations
- I can determine the direction a reaction will proceed by comparing Q to K, and recognize that when Q = K, the system is at dynamic equilibrium.
7.8 Representations of Equilibrium
- I can use particulate representations to describe the relative numbers of reactant and product particles present prior to and at equilibrium, and relate them to the value of the equilibrium constant.
7.9 Introduction to Le Châtelier’s Principle
- I can predict the response of a system to stresses such as addition or removal of a chemical species, change in temperature, change in volume/pressure, or dilution using Le Châtelier’s principle.
- I can predict the effect that a stress will have on experimentally measurable properties such as pH, temperature, and color of a solution.
7.10 Reaction Quotient and Le Châtelier’s Principle
- I can explain that a disturbance to a system at equilibrium causes Q to differ from K, and that the system responds by bringing Q back into agreement with K.
- I can identify that changes in concentration change Q only, while changes in temperature change K, and describe how species redistribute to equalize Q and K.
7.11 Introduction to Solubility Equilibria
- I can describe the dissolution of a salt as a reversible process using the solubility-product constant, Ksp.
- I can calculate the solubility of a substance from its Ksp and use this to predict the relative solubility of different substances.
- I can relate solubility rules to Ksp, recognizing that Ksp values >1 correspond to soluble salts.
7.12 Common-Ion Effect
Equilibrium: common questions
What is in Unit 7: Equilibrium?
It covers 12 topics: 7.1 Introduction to Equilibrium; 7.2 Direction of Reversible Reactions; 7.3 Reaction Quotient and Equilibrium Constant; 7.4 Calculating the Equilibrium Constant; 7.5 Magnitude of the Equilibrium Constant; 7.6 Properties of the Equilibrium Constant; 7.7 Calculating Equilibrium Concentrations; 7.8 Representations of Equilibrium; 7.9 Introduction to Le Châtelier’s Principle; 7.10 Reaction Quotient and Le Châtelier’s Principle; 7.11 Introduction to Solubility Equilibria; 7.12 Common-Ion Effect.
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